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Questions and Answers
Does all life require the same essential elements?
Does all life require the same essential elements?
False (B)
Which of the following is a chemical reaction?
Which of the following is a chemical reaction?
- Making a hydrogen bond between a water molecule and a sugar molecule
- Dissolving a lump of sugar in a cup of coffee
- Melting ice
- None of the above (correct)
What is the BEST explanation of what has occurred when Carbon-14 decays?
What is the BEST explanation of what has occurred when Carbon-14 decays?
- An ionic bond has formed
- The resulting atom is still carbon-14
- The resulting atom still has an unstable nucleus
- The resulting atom is now a different element because the number of protons has changed (correct)
What happens when two atoms form a chemical bond?
What happens when two atoms form a chemical bond?
What do you predict to be the charge on ammonium?
What do you predict to be the charge on ammonium?
How many electron pairs are shared between carbon atoms in a molecule that has the formula C2H2?
How many electron pairs are shared between carbon atoms in a molecule that has the formula C2H2?
What is a compound?
What is a compound?
Which bond or interaction would be difficult to disrupt when compounds are put into water?
Which bond or interaction would be difficult to disrupt when compounds are put into water?
Cations have a _________ charge and anions have a _________ charge.
Cations have a _________ charge and anions have a _________ charge.
A covalent bond is likely to be polar when:
A covalent bond is likely to be polar when:
Define electronegative.
Define electronegative.
Define element.
Define element.
Define essential elements.
Define essential elements.
Define trace elements.
Define trace elements.
What is carbon's atomic number and mass number?
What is carbon's atomic number and mass number?
What is an allotrope?
What is an allotrope?
What is oxygen's atomic number and mass number?
What is oxygen's atomic number and mass number?
Define atom.
Define atom.
What does the atomic number tell you?
What does the atomic number tell you?
What does the mass number tell you?
What does the mass number tell you?
Define ion.
Define ion.
Define isotope.
Define isotope.
Define radioisotopes.
Define radioisotopes.
What is radiocarbon dating - C14 used for?
What is radiocarbon dating - C14 used for?
The first electron shell can hold ___ electrons, the second and third electron shells can hold ___ electrons.
The first electron shell can hold ___ electrons, the second and third electron shells can hold ___ electrons.
What is the valence shell?
What is the valence shell?
What is a valence number?
What is a valence number?
Define molecule.
Define molecule.
When electron shells are full, atoms are ________.
When electron shells are full, atoms are ________.
When electron shells are not full, ______________ occurs.
When electron shells are not full, ______________ occurs.
What are the three types of chemical bonds?
What are the three types of chemical bonds?
Define ionic bonds.
Define ionic bonds.
Define covalent bonds.
Define covalent bonds.
Define polar covalent bonds.
Define polar covalent bonds.
Define non-polar covalent bonds.
Define non-polar covalent bonds.
Any bond between two atoms of the same element forms a _________ bond.
Any bond between two atoms of the same element forms a _________ bond.
Define free radical.
Define free radical.
What can you do to prevent free radical damage?
What can you do to prevent free radical damage?
Define hydrogen bonds.
Define hydrogen bonds.
Are hydrogen bonds strong?
Are hydrogen bonds strong?
List the three chemical bonds (ionic, hydrogen, and covalent) in order from strongest to weakest.
List the three chemical bonds (ionic, hydrogen, and covalent) in order from strongest to weakest.
Chemical bonds hold _________________ together and store __________.
Chemical bonds hold _________________ together and store __________.
Chemical equations describe _____________ ____________.
Chemical equations describe _____________ ____________.
In a chemical equation, reactants are written to the _______ of the arrow and products are written to the _______ of the arrow.
In a chemical equation, reactants are written to the _______ of the arrow and products are written to the _______ of the arrow.
Define oxidation.
Define oxidation.
Define reduction.
Define reduction.
An example of an oxidation-reduction reaction is ____________.
An example of an oxidation-reduction reaction is ____________.
Two examples of redox in biological systems are _________ and __________ _____________.
Two examples of redox in biological systems are _________ and __________ _____________.
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Study Notes
Essential Concepts in Chemistry
- All living organisms require essential elements, but not all share the same elements.
- A chemical reaction involves changes in molecular structure, unlike processes like dissolving or melting.
Carbon-14 and Nuclear Transitions
- Carbon-14, with 6 protons and 8 neutrons, is pivotal in carbon dating.
- When a neutron converts to a proton, it changes the atom's identity, indicating a transformation into a distinct element.
Chemical Bonds
- Atoms form chemical bonds by transferring or sharing outer electrons to achieve stable configurations.
- Nitrogen, typically forming three bonds, has a +1 charge in ammonium due to forming four bonds with hydrogen.
Covalent and Ionic Bonds
- Carbon in C2H2 shares three pairs of electrons through covalent bonds.
- Covalent bonds, particularly those between carbon atoms, are resistant to disruption in water.
- Cations carry a positive charge, while anions carry a negative charge.
Bond Polarities
- A covalent bond becomes polar if one atom is more electronegative than the other, leading to an unequal sharing of electrons.
- Electronegativity refers to an atom's tendency to attract electrons.
Elements and Structures
- Elements cannot be broken down by ordinary chemical reactions and have unique properties, defined by their atomic structures.
- Essential elements like oxygen, carbon, hydrogen, and nitrogen are crucial for life, while trace elements are needed in minute quantities.
Atomic Structure and Isotopes
- The atomic number indicates the number of protons, and the mass number combines protons and neutrons.
- Isotopes of an element differ in neutron count, with unstable radioisotopes undergoing decay.
Chemical Stability and Valence
- Atoms are stable when their electron shells are full; interactions occur when they are not.
- The valence shell determines an atom's chemical properties, and the valence number indicates electrons needed for stability.
Types of Chemical Bonds
- Chemical bonds include ionic, covalent, and hydrogen bonds, arranged from strongest to weakest as: covalent > ionic > hydrogen.
- Ionic bonds result from the attraction of oppositely charged ions, while covalent bonds involve shared electrons.
Molecular and Atomic Interactions
- A molecule comprises two or more atoms held together by electron interactions.
- Free radicals, which have unpaired electrons, are unstable and reactive, leading to potential cellular damage.
Reactions and Equations
- Chemical equations depict reactions, with reactants on the left and products on the right.
- Oxidation involves losing electrons, while reduction refers to gaining electrons. An example of a redox reaction is rusting.
Biological Significance
- Processes like glycolysis and cellular respiration demonstrate oxidation-reduction reactions in biological systems, highlighting their importance in metabolism.
Protective Measures
- To combat free radical damage, antioxidants such as vitamins A and E can be beneficial.
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